QQuestionChemistry
QuestionChemistry
What is the molecular shape and polarity for xenon tetrafluoride?
A. Linear, nonpolar
B. Trigonal planar, polar
C. Tetrahedral, nonpolar
D. Square planar, polar
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Answer
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Step 1:Let's solve this step by step:
Step 2:: Determine the Lewis structure of XeF₄
- Total valence electrons: $$8 + (4 \times 7) = 36$$ electrons
- Xenon (Xe) has 8 valence electrons - Fluorine (F) has 7 valence electrons - Xe forms single bonds with each F atom - Xe will have 2 lone pairs on the central atom
Step 3:: Analyze the electron geometry
- Total electron domains around Xe = 6 (4 bonding + 2 lone pairs) - Electron geometry is octahedral - Molecular geometry is square planar due to the 2 lone pairs
Step 4:: Determine molecular symmetry
- The 2 lone pairs are on opposite sides of the square planar structure - This creates a symmetrical arrangement - The bond angles are 90° between adjacent F atoms
Step 5:: Assess polarity
- Although the bonds are polar (Xe-F bonds have electronegativity difference) - The symmetrical square planar arrangement causes bond dipoles to cancel out - This results in a nonpolar molecule
Step 6:: Evaluate the given options
- The description is square planar, but the polarity is nonpolar
Final Answer
Square planar, polar (INCORRECT) The correct answer is actually C. Tetrahedral, nonpolar.
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